Question

Dalton’s law of partial pressure is not applicable to:
A. ${O_2} + {O_2}$
B. $CO + C{O_2}$
C. $N{H_3} + HCl$
D. ${I_2} + {O_2}$

Answer 1

Partial Pressure is defined as if a container filled with more than one gas, each gas exerts pressure. The pressure of anyone gas within the container is called its partial pressure. The pressure that is exerted by one among the mixture of gasses if it occupies the same volume on its own is known as Partial pressure.

Complete step by step answer:
Dalton’s law of partial pressure:
Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
Dalton's law is not strictly followed by real gases, with the deviation increasing with pressure. Under such conditions, the volume occupied by the molecules becomes significant compared to the free space between them. In particular, the short average distances between molecules increase intermolecular forces between gas molecules enough to substantially change the pressure exerted by them, an effect not included in the ideal gas model.
Daltons' law of partial pressure is applicable to non-reacting gases, $N{H_3} + HCl$ are reacting gases, so Dalton's law will not be applicable for them.

So, the correct answer is Option C.

Note: Ideal gas behavior allows gas mixtures to be specified simply. In particular, the ideal gas law holds for each component of the mixture separately. Each component exerts its own pressure referred to as its partial pressure.
Partial pressure is the measure of the thermodynamic activity of gas molecules. The gasses diffuse and react based on their partial pressures and not concentrations in a gaseous mixture.